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Question

The integrated rate equation for first-order reaction is $$A$$ $$\rightarrow$$ products.


A
K=2.303tlog[A]0[A]t
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B
K=1tln[A]t[A]0
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C
K=2.303tlog10[A]t[A]0
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D
K=1tln[A]t[A]0
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Solution

The correct option is A
$$K=\displaystyle\frac{2.303}{t}log\frac{[A]_0}{[A]_t}$$

For the first reaction, $$A$$ $$\rightarrow$$ Products, the integrated rate law is given by the equation.

$$K=\displaystyle\frac{2.303}{t}log\frac{[A]_0}{[A]_t}$$

where, 
$$[A]_0$$ is the initial concentration of the reactant at $$t=0$$

$$[A]_t$$ is the concentration of the reactant at t $$=$$ t.

So, the correct option is $$A$$.

Chemistry

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